A chemist dissolves 0.20 mol NH₃(g) in enough water to make 1.0 L of solution
CHEMISTRY · Single correct · A Level · Chemistry · Acids and bases · Acids and bases
Problem
A chemist dissolves 0.20 mol NH₃(g) in enough water to make 1.0 L of solution, then bubbles in 0.010 mol HCl(g) until it is completely dissolved. Which statement best describes the resulting solution?
(a) It will act as a buffer because appreciable amounts of both NH3 and NH4+ are present.
(b) It will not act as a buffer because the 19:1 ratio of weak base to conjugate acid is too large for buffering.
(c) It will act as an effective buffer against added strong acid, but not against added strong base.
(d) It will not act as a buffer because the strong acid forms NH4Cl, a salt that cannot buffer.